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Difference between revisions of "Bound energy"

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{{MitoPedia
{{MitoPedia
|abbr=''B'' [J]
|abbr=''B'' [J]
|description=The '''bound energy''' change in a closed system is that part of the [[energy]] change that is always bound to an exchange of [[heat]],
|description=The '''bound energy''' change in a closed system is that part of the ''total'' [[energy]] change that is always bound to an exchange of [[heat]],


ย  โˆ†''B'' = โˆ†''U'' - โˆ†''A'' [Eq. 1]
ย  d''B'' = d''U'' - d''A'' [Eq. 1]


ย  โˆ†''B'' = โˆ†''H'' - โˆ†''G'' [Eq. 2]
ย  โˆ†''B'' = โˆ†''H'' - โˆ†''G'' [Eq. 2]


The ''free'' energy change (Helmoltz or Gibbs; โˆ†''A'' or โˆ†''G'') is the ''total'' energy change (total inner energy or enthalpy, โˆ†''U'' or โˆ†''H'') of a system minus the ''bound'' energy change.
The ''free'' energy change (Helmoltz or Gibbs; d''A'' or d''G'') is the ''total'' energy change (total inner energy or enthalpy, d''U'' or d''H'') of a system minus the ''bound'' energy change.


Therefore, if a process occurs at [[equilibrium]], when โˆ†''G'' = 0, then โˆ†''H'' = โˆ†''B'', and at โˆ†<sub>e</sub>''W'' = 0 (โˆ†''H'' = โˆ†<sub>e</sub>''Q'' + โˆ†<sub>e</sub>''W''; see [[energy]]) we obtain the definition of the bound energy as the heat change taking place in an equilibrium process (eq),
Therefore, if a process occurs at [[equilibrium]], when d''G'' = 0 (at constant gas pressure), then d''H'' = d''B'', and at d<sub>e</sub>''W'' = 0 (d''H'' = d<sub>e</sub>''Q'' + d<sub>e</sub>''W''; see [[energy]]) we obtain the definition of the bound energy as the heat change taking place in an equilibrium process (eq),


ย  โˆ†''B'' = ''T''โˆ™โˆ†''S'' = โˆ†<sub>e</sub>''Q''<sub>eq</sub> [Eq. 3]
ย  d''B'' = ''T''โˆ™d''S'' = d<sub>e</sub>''Q''<sub>eq</sub> [Eq. 3]
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::::::* IUPAC: Helmholtz energy, ''A'' = ''U'' - ''TS'' [J]
::::::* IUPAC: Helmholtz energy, ''A'' = ''U'' - ''TS'' [J]
::::::* http://www.eoht.info/page/On+the+Thermodynamics+of+Chemical+Processes 2018-12-27 ย 
::::::* http://www.eoht.info/page/On+the+Thermodynamics+of+Chemical+Processes 2018-12-27 ย 
::::* Recalling the term ''bound energy'' helps to resolve one of the historic battles in thermodynamics [2]. ย 
::::* The term ''bound energy'' helps to resolve one of the historic battles in thermodynamics [2]. ย 


== References ==
== References ==

Latest revision as of 14:05, 31 December 2018


high-resolution terminology - matching measurements at high-resolution


Bound energy

Description

The bound energy change in a closed system is that part of the total energy change that is always bound to an exchange of heat,

dB = dU - dA [Eq. 1]
โˆ†B = โˆ†H - โˆ†G [Eq. 2]

The free energy change (Helmoltz or Gibbs; dA or dG) is the total energy change (total inner energy or enthalpy, dU or dH) of a system minus the bound energy change.

Therefore, if a process occurs at equilibrium, when dG = 0 (at constant gas pressure), then dH = dB, and at deW = 0 (dH = deQ + deW; see energy) we obtain the definition of the bound energy as the heat change taking place in an equilibrium process (eq),

dB = Tโˆ™dS = deQeq [Eq. 3]

Abbreviation: B [J]

History

  • From Kubo 1976 North-Holland: "Free energy" is due to H. van Helmholtz (1882), and means that part of the internal energy that can be converted into work, as seen in the equation dF = dA for an isothermal quasi-static process. It was customary to call the remaining part, TdS, of the internal energy, dU = dF+TdS, the gebundene Energie (bound energy), but this is not so common now.
  • The term bound energy helps to resolve one of the historic battles in thermodynamics [2].

References

  1. Kubo R (1976) Thermodynamics. An advanced course with problems and solutions. North-Holland Amsterdam, New York. -
  2. Gnaiger E (1994) Negative entropy for living systems: controversy between Nobel Laureates Schrรถdinger, Pauling and Perutz. In: What is Controlling Life? (Gnaiger E, Gellerich FN, Wyss M, eds) Modern Trends in BioThermoKinetics 3. Innsbruck Univ Press: 62-70. - ยปBioblast linkยซ


MitoPedia concepts: Ergodynamics